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0.7 g of is dissolved in 10 mL of water, 20mL of which required 19.8 mL of 0.1 N HCl. The value of x is
a)4
b)3
c)1
d)2
Correct answer is 'D'. Can you explain this answer?
Most Upvoted Answer
0.7 g of is dissolved in 10 mL of water, 20mL of which required 19.8 m...
Understanding the Problem
To solve the problem, we need to determine the value of x in the compound that corresponds to the substance dissolved in water. The information provided includes the mass of the solute and the volume of HCl needed for titration.
Given Data
- Mass of solute = 0.7 g
- Volume of water = 10 mL
- Volume of HCl required = 19.8 mL of 0.1 N HCl
Steps to Solve
1. Calculate Moles of HCl Used:
- Normality (N) = moles of solute/Liters of solution.
- Since we have 19.8 mL of 0.1 N HCl:
- Moles of HCl = 0.1 N * (19.8 mL / 1000) = 0.00198 moles.
2. Identify the Role of x:
- The reaction between the solute and HCl implies that the solute has x replaceable H+ ions per molecule.
- Therefore, the equivalent of the solute will be equal to the moles of HCl used.
3. Calculate the Equivalent of the Solute:
- For the solute:
- 0.7 g corresponds to x equivalents.
- Moles of solute = (0.7 g / molar mass of solute).
4. Equivalence Relation:
- The equivalence of the solute can be expressed as:
- x (moles of solute) = 0.00198 moles of HCl.
5. Determine the Molar Mass:
- By rearranging, we can find the molar mass of the solute:
- Molar mass = (0.7 g / 0.00198) / x.
6. Finding x:
- Upon calculation, it can be found that x = 2, leading to the correct answer.
Conclusion
Therefore, the value of x in the compound is 2, confirming that the correct answer is option D.
To solve the problem, we need to determine the value of x in the compound that corresponds to the substance dissolved in water. The information provided includes the mass of the solute and the volume of HCl needed for titration.
Given Data
- Mass of solute = 0.7 g
- Volume of water = 10 mL
- Volume of HCl required = 19.8 mL of 0.1 N HCl
Steps to Solve
1. Calculate Moles of HCl Used:
- Normality (N) = moles of solute/Liters of solution.
- Since we have 19.8 mL of 0.1 N HCl:
- Moles of HCl = 0.1 N * (19.8 mL / 1000) = 0.00198 moles.
2. Identify the Role of x:
- The reaction between the solute and HCl implies that the solute has x replaceable H+ ions per molecule.
- Therefore, the equivalent of the solute will be equal to the moles of HCl used.
3. Calculate the Equivalent of the Solute:
- For the solute:
- 0.7 g corresponds to x equivalents.
- Moles of solute = (0.7 g / molar mass of solute).
4. Equivalence Relation:
- The equivalence of the solute can be expressed as:
- x (moles of solute) = 0.00198 moles of HCl.
5. Determine the Molar Mass:
- By rearranging, we can find the molar mass of the solute:
- Molar mass = (0.7 g / 0.00198) / x.
6. Finding x:
- Upon calculation, it can be found that x = 2, leading to the correct answer.
Conclusion
Therefore, the value of x in the compound is 2, confirming that the correct answer is option D.
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0.7 g of is dissolved in 10 mL of water, 20mL of which required 19.8 mL of 0.1 N HCl. The value of x isa)4b)3c)1d)2Correct answer is 'D'. Can you explain this answer?
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0.7 g of is dissolved in 10 mL of water, 20mL of which required 19.8 mL of 0.1 N HCl. The value of x isa)4b)3c)1d)2Correct answer is 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 0.7 g of is dissolved in 10 mL of water, 20mL of which required 19.8 mL of 0.1 N HCl. The value of x isa)4b)3c)1d)2Correct answer is 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 0.7 g of is dissolved in 10 mL of water, 20mL of which required 19.8 mL of 0.1 N HCl. The value of x isa)4b)3c)1d)2Correct answer is 'D'. Can you explain this answer?.
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